In a 1.0× 10–4 M solution of HClO(aq), identify the relative molar amounts of these species from most to least: HClO, OCl, OH^-, H30^+, H20
To determine the relative molar amounts of the species in a 1.0 x 10^-4 M solution of HClO(aq), we need to consider the dissociation reaction of HClO. HClO partially dissociates in water to form H+ and ClO-.
The equation for the dissociation of HClO is as follows:
HClO ⇌ H+ + ClO-
Let's break down the relative molar amounts of the species based on the given information from most to least:
1. HClO:
In the given solution, the concentration of HClO is 1.0 x 10^-4 M. This means that for every 1 liter of the solution, we have 1.0 x 10^-4 moles of HClO. Therefore, the molar amount of HClO is 1.0 x 10^-4.
2. ClO- (OCl):
For every mole of HClO that dissociates, one mole of ClO- (or OCl) is formed. So, the molar amount of ClO- is also 1.0 x 10^-4.
3. H+ (H3O+):
Since HClO acts as an acid and donates a proton (H+) in its dissociation, the molar amount of H+ (or H3O+) is also 1.0 x 10^-4.
4. OH-:
In water, the concentration of OH- ions can be determined by the concentration of H+ ions (from H3O+ ions) based on the self-ionization of water. The self-ionization of water is as follows:
H2O ⇌ H+ + OH-
In pure water at 25°C, the concentration of H+ is equal to the concentration of OH-, which is 1.0 x 10^-7 M. However, in the presence of the H3O+ ions from the acid dissociation, the concentration of OH- will be extremely small compared to 1.0 x 10^-7 M. So, in this case, the molar amount of OH- can be considered negligible compared to the other species.
To summarize the relative molar amounts from most to least:
HClO = 1.0 x 10^-4
OCl- = 1.0 x 10^-4
H+ (or H3O+) = 1.0 x 10^-4
OH- = negligible compared to other species